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- What are theconsequences of shifting thechemical equilibrium of theformation of bicarbonate fromcarbon dioxide and watertowards the consumption ofproducts of the reversereaction?Showing the workings, estimate the lower flammability limit of tetrahydrofuran tetrahydrofuranWrite a balanced single-replacement reaction that is consistent with the above observations.
- Question: In the context of chemical reactions, explain the concept of kinetic versus thermodynamic control and provide an example to illustrate the difference. .Bromine in methylene chloride is added in stoichiometric proportions to cyclopentane. What color is the final solution? Group of answer choices clear orange purple yellow precipitate brown precipitate Bromine in methylene chloride is added in stoichiometric proportions to cyclohexa-1,3-diene. What color is the final solution? Group of answer choices clear orange purple yellow precipitate brown precipitate What does the 'N' in SN1 and SN2 stand for?What is meant by non-stoichiometric defect? Ionic solids which have anionicvacancies due to metal excess defect develop colour. Explain with the helpof suitable example.
- Compounds Mass 3-nitrophthalic acid used 200 mg = 0.2g 8% aqueous hydrazine used 0.4mL 3-nitrophthalhydrazide obtained 130 mg = 0.13 g sodium hydrosulfite dihydrate 0.6 g luminol obtained 70 mg = 0.07 g compute yield for nitrophthalhydrazide in the first step (assume nitrophthalic acid is limiting reagent) compute yield for luminol in the second step (using nitrophthalhydrazide as limiting reagent) compute yield for the overall reactionIn preparation of dibenzalacetone, what is limiting factor?fischer esterification: 5.4mL of isopentyl alcohol, molar mass 88.15g/mol: 8.5mL of acetic acid, molar mass 60.05 g/mol: Experimental final product(Isopentyl acetate) I got: 3.10g. 1.Calculate for theretical yield. 2.Percentage yield 3. % recovery.
- 1. Write three major criteria of forming a Hydrogen bond in bullet points with example. 2. Certain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed the exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 5 kg of nitrogen gas was found, calculate the amount of charcoal used. (12C, 16O, 14N)b. Compound 4.2 was reacted with Br₂ in H₂O and three compounds were observed after completion of the following reaction: CH3 4.2 Br₂ H₂O Table 4.1 summarises the yield and molecular formula of the products (Compounds 4.3, 4.4 and 4.5). 4.4 Table 4.1: The yields of Compounds 4.3, 4.4 and 4.5. Compound 4.3 4.5 Yield/% 90 4.3, 4.4 and 4.5 8 2 Molecular formula C11H13 OBr C11H13OBr C11H12Br2ASSume an excesS of of Zn? t Iz fac) +Zn Iz faa) 2.